In a first order reaction,the concentration of the reactant is reduced to $25\%$ in one hour. The half-life period of the reaction is:

For a first-order reaction,the half-life period is $69.3 \ s$. If the concentration of the reactant is $0.10 \ mol \ L^{-1}$,what will be the rate of the reaction?

Time required to decompose $SO_2Cl_2$ to half of its initial amount is $40 \ minutes$. If the decomposition is a first order reaction,what will be the rate constant of the reaction?

For a first order reaction $A \rightarrow B$, the data is provided in the table below. Find $x$ in minutes. (Nearest integer)

$t/\text{min}$	$[A]/M$
$0$	$0.6500$
$x$	$0.0650$
$20$	$0.00065$

For a first order reaction,the time required for completion of $90 \%$ reaction is '$x$' times the half life of the reaction. The value of '$x$' is $........$. (Given: $\ln 10 = 2.303$ and $\log 2 = 0.3010$)

Calculate the amount of reactant in percent that remains after $60 \ min$ in a first-order reaction. $(k = 0.02303 \ min^{-1})$ (in $\%$)